Final Exam Review Multiple-Choice Questions Combined1. Use the VSEPR theory to predict molecular geometry of IF5.a) tetrahedralb) see-saw

c) trigonal bipyramidald) square pyramidal

e) octahedral

2. Use the VSEPR theory to predict molecular geometry of CO32-.

a) bentb) tetrahedral

c) trigonal pyramidald) T-shaped

e) trigonal planar

3. What is the bond angle between the O-N-O bonds in NO2- ion?a) 180 b) 120 c) 118 d) 90 e) 88

4. What is the molecular shape of SeO3?a) see-sawb) trigonal pyramidal

c) trigonal planard) tetrahedral

e) T-shaped

5. What is the molecular shape of the SF3- ion?

a) linearb) bent

c) trigonal planard) tetrahedral

e) T shaped

6. For XeF4, the valance electron geometry around the central atom is _____.a) trigonal planarb) tetrahedral

c) trigonal bipyramidald) octahedral

e) square planar

7. The molecular shape for XeF4 is _____.a) trignoal planarb) tetrahedral

c) trigonal bipyramidald) octahedral

e) square planar

8. The F-Xe-F bond angle in XeF4 molecule is _____.a) 90b) 109.5

d) 180

e) none of these

For the following 4 questions, the following molecular substances are referred to. Any substance may be used more than once in answering the questions. CO2, SO2, SiF4, XeF4

9. The species which has tetrahedral as the valence electron geometry is ____.a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

10. The species which has linear molecular geometry is ____.a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

11. The species which is polar is ____.a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

12. The species which has two lone pairs of valence electrons on the central atom is ___.a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

13. The species which bond angle is close to 120 degrees is ___.

a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

14. The species which bond angle is 109.5 degrees is ___.a) CO2 b) SO2 c) SiF4 d) XeF4 e) none of these

15. A polar molecule is one in which there is a separation of charge caused by ____.a) an average distribution of electronsb) a non-uniform electron distribution

c) a complete loss of electronsd) an uneven number of electron pairs

16. Which of the following is <strong>not</strong>a polar molecule?a) hydrogen chlorideb) hydrogen

c) waterd) ammonia (NH3)

17. Identify the formula which represents a nonpolar molecule.a) HCl b) NH3 c) CF4 d) H2S e) Al2S3

18. Which represents a polar molecule?a) F2 b) O2 c) CH4 d) CO2 e) HCl

19. Which atom will form the most polar bond with hydrogen?a) F b) Cl c) Br d) I e) O

20. Why is NH₃ classified as a polar molecule?a) It is a gas at room temperature and 1 atmosphere pressure.b) N-H bonds are non-polar.c) Nitrogen and hydrogen are both nonmetals.d) NH₃ molecules have asymmetrical charge distributions.

21. Which represents a nonpolar molecule?a) H2 b) NH3 c) CF4 d) SO2

22. Which statement best explains why carbon tetrachloride (CCl4) is non-polar?a) Each carbon-chloride bond is polar.b) Carbon and chlorine are both nonmetals.c) Carbon tetrachloride is an organic compound.d) The carbon tetrachloride molecule is symmetrical so all the polar bonds cancel each other out.

23. The compound XeF4 is _____.a) ionic b) polar c) nonpolar d) none of these

24. Which is an example of a nonpolar molecule that contains polar covalent bonds?a) CBr4 b) N2 c) H2 d) NH3

25. A solute is most likely to be highly soluble in a solvent if the solute is _____ and the solvent is ______.a) ionic or polar, polarb) ionic or polar, nonpolar

c) nonpolar, polard) nonpolar, ionic

26. Why is the normal boiling point of hydrogen fluoride is so much higher than that of hydrogen chloride, the hydride of the next element in group 17?a) The electron cloud in the HF molecule is more easily distorted (i.e. is more polarizable) than that of HCl.b) The HF molecules undergoes a higher degree of hydrogen bonding than HCl.c) HCl molecules are non-polar.d) The HF molecules have a lower dipole moment.e) Chlorine in HCl is more electronegative than fluorine in HF.

27. The boiling point of CH4 is much lower than that of HF. This is because: a) HF is more polarizable.b) of hydrogen bonding in HF.c) of ion-dipole interactions in CH4.

d) of dipole-dipole interactions in CH4.e) CH4 is polar.

28. The vapor pressure of a liquid increases exponentially with increasing temperature chiefly because ____.a) the enthalpy of vaporization increasesb) atmospheric pressure increasesc) the average molecular mass increasesd) the fraction of high energy molecules increases much faster than the average energye) the strength of the intermolecular forces increases

29. At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is a solid. This is because ______.a) dispersion interactions increase with molecular sizeb) dipole-induced dipole interactions increase with molecular sizec) dipole-dipole interactions increase with molecular sized) polarity increases with molecular sizee) dispersion interactions increase with molecular size and polarity increases with molecular size

30. Molecular iodine would be most soluble in ____.a) waterb) carbon tetrachloridec) vodka (ethanol and water)

d) vinegar (acetic acid and water)e) equally soluble in all four

31. The concept of "like dissolves like" is illustrated by which of the following? a) CuSO4(s) is more soluble in CCl4 than in water.b) NaCl (s) is more soluble in CCl4 than in water.c) I2(s) is more soluble in CCl4 than in water.d) CCl4 is soluble in water.e) I2(s) is more soluble in water than in CCl4.

32. For a given substance, which of the following phase transitions should RELEASE the most energy?a) Solid to liquid.b) Gas to solid.

c) Solid to gas.d) Liquid to gas.

e) Gas to liquid.

33. The boiling point of water is about 200°C higher than one would predict from the boiling points of hydrogen sulfide and hydrogen selenide. One may explain this apparent anomaly by which of the following?

a) Water is less polar than hydrogen sulfide and hydrogen selenide.b) Water has the lowest molecular weight.c) The H-O covalent bond is much stronger than the H-S and H-Se bonds.d) The water molecule is lighter than the other two molecules.e) The intermolecular attractive forces are much greater in water than in hydrogen sulfide and hydrogen selenide.

Based on the following information:CF4, Molecular Weight 87.99, Normal Boiling Point -182°CCCl4, Molecular Weight 153.8, Normal Boiling Point -123°C34. Which of the above substances would have the higher equilibrium vapor pressure assuming that both substances are in the liquid state at the same temperature?a) CF4

b) CCl4

c) CF4 and CCl4 would have the same vapor pressure.d) Impossible to determine from the information given

35. The intermolecular forces of attraction in the above substances is described by which of the following?a) Dipole-dipole forces (permanent dipoles).b) Gravitational forces.c) Repulsive forces.

d) Dispersion (or London) forces.e) Ion-dipole forces.

36. State why the normal melting point of ICl (27.2°C) is so much higher than that of Br2 (-7.2°C). The molecules of both substances have the same number of electrons. a) The Cl atom in the ICl molecule is more polarizable than the Br atom in the Br2 molecule.b) The ICl molecules undergo hydrogen bonding.c) The ICl molecules have a lower molecular weight.d) ICl molecules are polar.e) Iodine in ICl is more electronegative than bromine in Br2.

37. One of the reasons that solid CuSO4 dissolves in water is ____.a) The ion-dipole forces between the ions and the water molecules.b) The electrostatic force of attraction between the Cu2+ and the SO4

2- ions.c) Instantaneous dipole-induced dipole forces (dispersion or London forces) between the Cu2+ and the SO4

2- ions.d) The hydrogen bonding between the water molecules.e) Instantaneous dipole-induced dipole forces (dispersion or London forces) between the water molecules.

38. When ice melts, ____.a) a phase change occurs from a solid phase to liquid phaseb) an endothermic process occurs which requires energyc) the water changes from a crystalline solid to a liquidd) the water molecules take on more kinetic energye) all of the above

39. When water freezes, _____.

a) a phase change occurs from a liquid phase to a solid phaseb) an exothermic process occurs where energy is lost from ice to the surroundingc) the liquid water changes froom a random structure to a crystalline solidd) water molecules reduce their kinetic energiese) all of the above

40. Solids have all of the following properties EXCEPT:a) a definite shapeb) a definite mass

c) a definite colord) a definite volume

e) all of the above

41. Liquids have all of the following properties EXCEPT:a) no definite shapeb) a definite mass

c) a definite shaped) a definite volume

e) all of the above

42. The following are all properties of gases EXCEPT:a) a definite volumeb) no definite shape

c) no definite volumed) no definite mass

e) all of the above

43. Which of the following is true as solid changes into a liquid during melting?a) Increase in particle order.b) Energy change is exothermic.c) Particles lose freedom.

d) Temperature stays constant.e) Decrease in kinetic energy for particles.

44. Which of the following is true when a liquid changes into a gas during boiling?a) Temperature rises.b) Increases in particle order.c) Particles gain freedom.

d) Energy change is exothermic.e) Decrease in particle kinetic energies.

45. Gases diffuse because they ____.a) easily move as convection currentsb) are made of rapidly moving particlesc) have low boiling points

d) have a low densitye) none of the above

46. Which of the following best describes what happens to the particles of water when it boils? a) They lose energy and escape into the atmosphere.b) They gain kinetic energy and increase their freedom to move without significant attraction.c) They lose energy and lose freedom to move about.d) They gain energy and gain freedom to move about.e) None of the above.

47. Which of the following is true as a gas is changing to a liquid in condensation?a) particles gain freedomb) energy change is exothermicc) decrease in particle orderd) temperature risese) increase in particle kinetic energy

48. Which is most effective in changing a gas into a liquid?

a) Reduce the temperature and pressure.b) Increase the temperature and pressure.c) Reduce the temperature and increase the pressure.d) Increase the temperature and reduce the pressure.e) Increase the temperature but hold the pressure constant.

49. The cooling effect accompanying the evaporation of a liquid is the result of ____.a) higher energy particles being added to the liquidb) lower energy particles being added to the liquidc) lower energy particles leaving the liquidd) higher energy particles leaving the liquide) all are correct

50. The temperature at which the vapor pressure of a liquid equals the existing atmospheric pressure at the surface of the liquid is called the ____.a) boiling point of the liquidb) equilibrium vapor pressure temperaturec) saturation point of the atomosphered) normal atomospheric temperaturee) dew point

51. The intermolecular forces in a liquid X are greater than those in a liquid Y. Comparing the two liquids, it could be expected that liquid X would have _____.a) the lower normal boiling temperatureb) the lower critical temperaturec) the lower vapor pressure at a given temperatured) the higher rate of evaporatione) no conclusions can be stated

52. Which is a basic assumption of the kinetic molecular theory?a) Particles are in random motion.b) Particles undergo inelastic collisions.c) Particles lose energy with an increase in velocity.d) Particles travel faster as the temperature decreases.e) Particles lose energy when the temperature increases.

53. Which statement best accounts for the fact that gases can be greatly compressed?a) Molecules occupy space.b) The collisions of molecules are elastic.c) The molecules of a given gas are identical.d) Molecules of gases are in constant motion.e) Molecules of gases are relatively far apart from each other.

54. A solute is most likely to be highly soluble in a solvent if the solute is _____ and the solvent is ______.a) non-polar, polarb) ionic or polar, non-polar

c) ionic or polar, polard) non-polar, ionic

e) ionic, non-polar

55. Which element is present in all organic compounds?a) Carbon.b) Nitrogen.

c) Oxygen.d) Phosphorous.

e) Chlorine.

56. Which property is generally characteristic of an organic compound?a) Low melting point.b) High melting point.

c) Soluble in polar solvents.d) Insoluble in nonpolar solvents.

e) None of these.

57. Which compounds are isomers?a) 1-propanol and 2-propanolb) methanoic acid and ethanoic acidc) methanol and methanal

d) ethane and ethanole) none of these

58. Which statement explains why the element carbon forms so many compounds?a) Carbon atoms combine readily with oxygen.b) Carbon atoms have very high electronegativity.c) Carbon readily forms ionic bonds with other carbon atoms.d) Carbon readily forms covalent bonds with other carbon atoms.e) None of these.

59. What is the name of the compound that has the molecular formula C₆H₆?a) butaneb) butene

c) benzened) butyne

e) none of these

60. In a molecule of CH₄, the hydrogen atoms are spatially oriented toward the centers of a regular ____.a) pyramid b) tetrahedron c) square d) rectangle e) octahedron

61. In which pair of hydrocarbons does each compound contain only one double bond per molecule?a) C2H2 and C2H6b) C2H2 and C3H6

c) C4H8 and C2H4d) C6H6 andC7H8

e) None of these pairs.

62. Which compound is a saturated hydrocarbon?a) Ethene b) Ethane c) Ethyne d) Ethanol

63. What is the maximum number of covalent bonds than an atom of carbon can form?a) 1 b) 2 c) 3 d) 4 e) 5

64. Which class of organic compounds can be represented as R -OH?a) acids b) alcohols c) esters d) ethers e) ketones

65. Which molecule contains a total of three carbon atoms?a) 2-methylpropaneb) 2-methylbutane

c) propaned) butane

e) pentane

66. What substance is made up of monomers joined together in long chains?a) ketone b) protein c) ester d) acid e) alcohol

67. Which compound is an organic acid?a) CH3OH b) CH3OCH3 c) CH3COOH d) CH3COOCH3

68. Which of the following statements is true regarding ethene?a) Both carbon atoms are sp2 hybridized and the molecule is planar.b) Both carbon atoms are sp2 hybridized and all bond angles are approximately 109.5˚.c) One carbon atom is sp hybridized while the other is sp2.d) Both carbon atoms are sp3 hybridized and all bond angles are approximately 109.5˚.e) Both carbon atoms are sp hybridized and the molecule is planar.

69. Which of the following compounds contains the greatest percentage of oxygen by weight?a) C3H6O5Cl b) C3H6O2 c) C5H10O5 d) C4H8O3 e) All are equal.

70. The first and simplest alkane is _____.a) ethane b) methane c) C2H2 d) methene e) CCl4

71. Compounds that have the same composition but differ in structural formulas are _____.a) used for substitution productsb) called polymersc) usually alkane

d) having the same propertiese) called isomers

72. Ethene is the first member of the ___.a) alkane seriesb) alkyne series

c) saturated hydrocarbonsd) unsaturated hydrocarbons

e) aromatic hydrocarbons

73. The characteristic group of the organic ester is ____.a) -CO- b) -COOH c) -CHO d) -O- e) -COO-

74. The double bond in alkenes have _____ hybridized orbitals.a) sp b) sp2 c) sp3 d) sp3d2 e) sp4d3

75. The multiple bond in alkyne can be best described as ____.a) Two sigma bonds and one pi bond.b) Two sigma bonds and one pi bond.c) One sigma bonds and two pi bonds.

d) Three sigma bonds.e) Three pi bonds.

76. sp2 hybridization will be found for carbon in ____.a) CH4 b) C2H4 c) C2H6 d) CH3OH e) CH3OCH3

77. The primary products of complete combustion of hydrocarbons are ____.a) water and carbonb) water and carbon monoxide

c) water and carbon dioxided) hydrogen and carbon monoxide

e) hydrogen and carbon dioxide

78. Which of the following statements is the best expression for the sp³ hybridization of carbon electrons?a) The new orbitals are one s orbital and three p orbitals.b) The s electron is promoted to the p orbitals.

c) The s orbital is deformed into a p orbital.d) Four new and equivalent orbitals are formed.e) The s orbital electron loses energy to fall back into a partially filled p orbital.

79. The structure of the third member of the alkyne series is ____.a) H—C≡C—Hb) H—C≡C—CH3

c) H—C≡C—CH2CH3

d) H—C≡C—C≡C—He) H—C—C—CH=C—H2

80. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will ______.a) decreaseb) increasec) remain the same

d) increase first then decrease

e) decrease first then increase

81. The phase change represented by the equation: I2(S) I2(g) is called _______.a) sublimation b) condensation c) melting d) boiling e) freezing

82. Under the same conditions of temperature and pressure, a liquid differs from a gas because the particles of the liquid _____.a) are in constant straight-line motionb) take the shape of the container they occupyc) have no regular arrangementd) have stronger forces of attraction between theme) None of these.

83. Which process releases heat as it occurs?a) Evaporation of water.b) Melting of snow.

c) Burning hydrogen in the air to make water.d) Condensation of steam into water droplets.

84. The heat of fusion is the heat energy required to convert _____.a) a solid to a gas b) a liquid to a gas c) a solid to a liquid d) a gas to a liquid

85. Which two processes involve the same heat change, but differ only in the direction of the flow of heat?a) freezing and meltingb) freezing and condensation

c) condensation and meltingd) melting and boiling

e) freezing and condensation

86. Heating a solid at its melting temperature ____.a) raises the temperature of the solidb) drives the change from solid to liquid

c) has no effectd) reverses the process

87. Sublimation is ____.a) conversion of a liquid to the vapor stateb) conversion of a solid directly to the vapor statec) conversion of a solid to a liquid immediately followed by heating the liquid to the boiling pointd) conversion of a liquid to the solid state

88. The graph below represents the heating curve of a substance that starts as a solid below its freezing point.

<img src="../X- Images/heating curve of a substance.png" alt="heating curve of a substance.png" title="heating curve of a substance" width="749" height="440" style="display: block; margin-left: auto; margin-right: auto; text-align: center;"></img>

What is the melting point of this substance?a) 30°C b) 55°C c) 90°C d) 120°C

89. The temperature above which gas molecules become to energetic to form a true liquid, no matter what the pressure, is called the ________.a) Melting point b) Critical point c) Boiling point d) Triple point

90. Which of the following processes can occur when the temperature of a substance is increased at constant pressure?

I. SublimationII. MeltingIII. Boiling

a) I only. b) II only. c) II and III. d) I, II, and III

91. During which of the following phase changes must heat be added to overcome intermolecular forces?I. VapoizationII. SublimationIII. Depositiona) I only.b) II only.

c) I and II only.d) II and III only.

e) I, II, and III.

92. The temperature change represented by one Kelvin degree compared to one Centigrade degree is ____.a) 273 times as greatb) 1/273 as great

c) identicald) 100 times as great

e) none of these

93. The expression “a cubic foot of air” is unsatisfactory because ______.a) air volume is negligibleb) air has a very low densityc) gas volume is dependent on its temperature

d) gas volume is difficult to measuree) the metric system is more exact

94. When the pressure of ammonia gas is increased at constant temperature, _____.a) the energy if the molecules increasesb) the spaces between molecules increasec) the bonds between atoms are broken

d) liquid ammonia formse) none of these

95. A toy balloon tends to become spherical when inflated because ______.a) gases exert pressure equally in all directionsb) the balloon contains carbon dioxidec) air tends to be permeable

d) the rubber used in balloons contains impuritiese) none of these reasons

96. Which of the following gas occupies the smallest volume?a) Gas A: 2 moles at 760 mm and 273 K. b) Gas B: 1 mole at 380 mm and 273 K.

c) Gas C: 1 mole at 760 mm and 273 K.d) Gas D: 2 moles at 760 mm and 546 K

e) Gas E: 3 moles at 760 mm and 546 K

97. A gas has a volume of 100 ml. at a temperature of 27˚C. At constant pressure, what volume does this gas occupy at standard temperature?a) 10.7 mL b) 81.9 mL c) 91.0 mL d) 109.9 mL e) 819.0 mL

98. If there is no change in pressure for a sample of gas at 25 ˚C, which temperature will cause an increase in volume of this gas?a) 248 K b) 298K c) 35˚F d) 310K e) none of these

99. Which gas contains molecules with the highest average kinetic energy?a) Gas A: 2 moles at 273 K.b) Gas B: 1 mole at 293 K.

c) Gas C: 1 mole at 500 K.d) Gas D: 2 moles at 546 K.

e) Gas E: 2 mole at 500 K.

100. Two moles of nitrogen gas are mixed with 3 moles of hydrogen gas at 273 K and placed in a 22.4 liter container. The pressure of this mixture of gases is ____.a) 4 atm b) 1 atm c) 5 atm d) 3 atm e) 6 atm

101. Which of the following gases would be the densest at standard temperature and pressure?a) Helium b) Argon c) Carbon dioxide d) Xeon e) Nitrogen

102. In the laboratory, a sample of hydrogen is collected by water displacement. The sample of hydrogen has a volume of 25 mL at 24.0˚C and a barametric pressure for the day of 758 mmHg. What is the pressure of the dry gas at this temperature? (The water vapor pressure at 24.0 ˚C is 22.4 mmHg.)a) 455 mmHg b) 470 mmHg c) 736 mmHg d) 758 mmHg e) 780 mmHg

103. A sample of dry air contains 210 mL of oxygen, 780 mL of nitrogen, and 10 mL of all other gases. What is the pressure in mm of Hg due to the nitrogen if the total pressure was 1000 mmHg?a) 1000 mmHg b) 780 mmHg c) 577 mmHg d) 210 mmHg e) None of these.

104. Which system contains molecules with the same average kinetic energy as the molecules in 10.0 grams of carbon dioxide at 100˚C?a) 10 grams if CO2 at 40˚C.b) 20 grams if CO2 at 20˚C.

c) 20 grams if CO2 at 5˚C.d) 40 grams if CO2 at 10˚C.

e) None of these.

105. At the same temperature and pressure, which gas diffuses most rapidly through a porous membrane?a) NH₃b) CO₂c) NOd) N₂e) O₂

106. A gas sample is at 350^oC. If the pressure remains unchanged, which temperature will cause a decrease in volume of this gas?a) 51^oFb) 38^oC

c) 308 Kd) 40 ^oCe) None of these.

107. The temperature of a sample of helium gas is a measure of its ____.a) kinetic and potential energyb) average potential energyc) average kinetic energy

d) total potential energye) average of kinetic and potential energy

108. If the level of the mercury column inside a eudiometer is one inch lower than the level of the mercury outside the eudiometer, the gas pressure inside the eudiometer is ________.a) equal to that of the atmosphereb) equal to barometric pressurec) less than barometric pressure

d) more than barometric pressuree) less than the atomsphere

109. A gas occupies a 1.5 liter container at 250^oC and 2.0 atmospheres. If the gas is transferred to a 3.0 liter container at the same temperature, what will be the new pressure?a) 1.0 atm b) 2.0 atm c) 3.0 atm d) 4.0 atm e) 5.0 atm

110. Doubling the initial pressure under which 1000 ml. of a gas was confined causes the volume of the gas to ________.a) doubleb) remain the same

c) decrease very slightlyd) decrease greatly

e) increase greatly

111. If the volume which a certain number of gas molecules occupies remains constant as the temperature is lowered, then the pressure exerted by this number of molecules ______.a) remains constantb) steadily decreasesc) steadily increases

d) first increases and then decreasese) first decreases and then increases

112. When a bottle of perfume is opened, its fragrance spreads quickly all over a room. This is an example of _____.a) molarity b) compressibility c) diffusion d) expansibility e) ductility

113. Equal volumes of ideal gases contain the same number of molecules, provided the gases have equal _____.a) massesb) pressuresc) temperatures

d) temperatures and pressurese) masses and temperatures

114. The volume of a certain amount of dry gas is inversely proportional to the pressure, provided the temperature remains constant. This Law is credited to ____.a) Charles b) Boyle c) Kelvin d) Bohr e) Avgardro

115. Hydrogen is collected by water displacement. The water levels in the bottle and the pneumatic trough are made equal. The barometric pressure is 723.2 mmHg and the vapor pressure is 19.8mmHg. What is the pressure of the H2 collected and what must be measured to determine the mass of H2 collected?

a) 703.4 mm; the volume of H2 must be determined.b) 703.4 mmHg; nothing else is needed.c) 740.0 mmHg; the volume of H2 must be determined.d) 740.0 mmHg; the Celsius temperature must be converted to Kelvin.e) 723.2 mmHg; the moles of H2 must be determined.

116. Nitrogen is collected in a gas tube over water. The water level inside the tube is 28.6 mm lower that that outside. The barometric pressure that day is 770 mmHg. The water vapor pressure at the room temperature of 22^oC is 19.8 mmHg. What is the pressure of the dry nitrogen?a) 721.6 mmHgb) 761.2 mmHgc) 778.8 mmHgd) 792.4 mmHge) 818.4 mmHg

117. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?a) It is equal to 1/3 the total pressure.b) It depends on the intermolecular forces of attraction between molecules of X, Y and Z.c) It depends on the relative molecular masses of X, Y and Z.d) It depends on the average distance traveled between molecular collisions.e) It can be calculated with knowledge only of the volume of the container.

118. One mole of nitrogen, two moles of neon, and four moles of argon are sealed in a cylinder. The combined pressure of the gases is 1400 mm of Hg. What is the partial pressure of the nitrogen, in mm of Hg?a) 100 mm b) 200 mm c) 400 mm d) 500 mm e) 1,400 mm

119. A gas mixture contains twice as many moles of O₂ as N₂. Additions of 0.200 mole of argon to this mixture increases the pressure from 0.800 atm to 1.10 atm. How many moles of O₂ are in the mixture?a) 0.355 moleb) 0.178 mole

c) 0.533 moled) 0.200 mole

e) 0.0750 mole

120. If there are 7.0 x l0⁴ molecules of water vapor and 3.0 x 10⁶ molecules of CO₂ present in a container having a total pressure of 670 mmHg, what is the partial pressure of CO₂?a) 15 mmHg b) 90 mmHg c) 456 mmHg d) 564 mmHg e) 655 mmHg

121. If 3.4 moles of chlorine gas are added to 2.2 moles of fluorine gas at 136.5 K and placed in a 22.4 liter container, what is the pressure of this gas mixture?a) 2.8 atm b) 4.4 atm c) 5.6atm d) 6.8 atm e) 8.2 atm

122. Cooling a gas from 100^oC to a temperature of 0^oC causes its original volume to _____.a) remain unchangedb) be decreased by 100/373

c) be increased by 100/373d) be halvede) be doubled

123. Consider the reaction: NO + O₂ --> NO₂. If 6 liters of NO₂ gas (at STP) are formed according to the reaction, what volume of O₂ at 1 atm pressure and a temperature of 546 K must have been used?a) 1.0 L b) 1.5 L c) 3.0 L d) 4.8 L e) 6.0 L

124. If the density for the gas neon is 0.3 gram/liter, what volume will one mole of this gas occupy?a) 9.7 L b) 67.3 L c) 84.1 L d) 89.3 L e) 101 L

125. Which conditions generally cause the characteristics of a gas to deviate most from the ideal gas laws?a) High temperature and low pressure.b) High temperature and high pressure.c) Low pressure and low temperatured) Low temperature and high pressure.e) Low molecular masses and low volumes.

126. The diffusion rate of hydrogen, H₂, is 1600 meters/sec. Under similar conditions, what is the diffusion rate of oxygen, O₂?a) 19.89 m/sec

b) 400 m/secc) 100 m/sec

d) 600 m/sece) 6400 m/sec

127. How does the average kinetic energy of hydrogen molecules compare with that of oxygen molecules when both gases are at 25^oC?a) They have equal K.E. (kinetic energy).b) The K.E. of hydrogen is 1/4 as great.c) The K.E. of hydrogen is 1/16 as great.d) The K.E. of hydrogen is 4 times as great.e) More information is needed.

128. At constant temperature, the behavior of a sample of a real gas more closely approximates that of an ideal gas as its volume is increased because the ____.a) collisions with the walls of the container become less frequentb) average molecular speed decreasesc) molecules have expandedd) average distance between molecules becomes greatere) average molecular kinetic energy decreases

129. In which of the following is it impossible to predict whether the pressure of a gas will increase, decrease, or stay the same?a) A gas sample is heated.b) A gas sample is heated, and the volume is increased.c) A gas sample is cooled, and some gas is withdrawn.d) Additional gas is added to a sample of gas.

e) A gas sample is cooled, and the volume is increased.

130. Under the same conditions of temperature and pressure, which gas diffuses most rapidly?a) Arb) Hec) N₂d) CO₂e) SO₃

131. How many liters of propyne gas, C₃H₄, at 1,000 mmHg pressure and 273 K were used in a combustion reaction if 80 grams of water resulted from this reaction?a) 37.8 L b) 65.5 L c) 75.6 L d) 84.0 L e) 88.8 L

132. Which curve shows the relationship between the volume of an ideal gas (at constant pressure) and its temperature in degrees Kelvin?<img src="../X- Images/Q267.png" alt="Q267.png" title="Q267" width="488" height="137" style="display: block; margin-left: auto; margin-right: auto; text-align: center;"></img>a) 1 b) 2 c) 3 d) 4 e) 5

133. At constant pressure, which curve best shows the relationship between the volume of an ideal gas and its absolute temperature?<img src="../X- Images/Q268.png" alt="Q268.png" title="Q268" width="248" height="113" style="display: block; margin-left: auto; margin-right: auto; text-align: center;"></img>a) Ab) B

c) Cd) D

e) None of these.

134. At constant pressure density, D, of a gas sample is inversely proportional to the absolute temperature, T. Which of the following is a graph of the relation of the density of a gas sample to the absolute temperature if the pressure is constant?<img src="../X- Images/Q269.png" alt="Q269.png" title="Q269" width="680" height="70" style="display: block; margin-left: auto; margin-right: auto; text-align: center;"></img>a) 1b) 2c) 3d) 4e) 5

135. In a balanced chemical equation, ______.a) coefficients are equalb) atoms are conservedc) molecules are equald) energy is always producede) none of those

136. Which of the following statement about a chemical reaction is <strong>FALSE</strong>?a) The mass of the reactants consumed equals the mass of the products formed.b) No atoms are created nor destroyed in the reaction.

c) The number of molecules of products equals the number of molecules of reactants.d) The reaction produces new moleucles through rearrangement of atoms.

137. To satisfy the law of conservation of mass, a chemical equation _____.a) must be written in wordsb) should show the atomic mass of both reactants and productsc) must be balancedd) must indicate the physical state of each of the reactants and products

138. The number of atoms of oxygen indicated by the formula 3Ca₃(PO₄)₂ is a) 24b) 12c) 8d) none of those.

139. Which of the following expressions represents two molecules of water?a) H₂Ob) H₂O₂c) 2H₂Od) 2HO₂e) None of these.

140. The breakdown of a complex substance to form two or more simpler substance is:a) decompositionb) composition

c) replacement d) double-replacement

141. The substances to the left of the arrow in a chemical equation are calleda) coefficients. b) prducts. c) subscripts. d) reactants.

142. In every balanced chemical equation, one should find represented on both sides the same number of ____.a) atoms b) coefficients c) isotopes d) molecules

143. A gas whose molecule is monatomic is ____.a) oxygen b) helium c) nitrogen d) chlorine e) hydrogen

144. C + O₂ ---> CO₂ means which of the following?a) Calcium and ozone will react and form a stable compound.b) When carbon combines with oxygen, carbon dioxide is produced.c) Carbon monoxide is released when gasoline is burned.d) The air contains two molecules of oxygen and one of carbon.

145. A hypothetical element Z forms a chloride with the formula ZCl₅. What is the most probable formula for its oxide?a) ZO₂b) ZO₅c) Z₂O₅

d) Z₅O₂

146. When a correctly written formula equation is balanced, ____a) the total number of atoms on one side must equal to the total number of atoms of the other side.b) the sum of the coefficients on the left side must equal to the coefficients sum on the other side.c) the number of subscripts on each side must be equal.d) all molecules must be diatomic.

147. A word equation states all of the following <strong>except</strong>:a) the substances which enter into the chemical reaction.b) the substances which are produced by a chemical reaction.c) the quantities of substances involved.d) an experimental fact or facts.

148. The process whereby a chemist produces a new compound by combining elements or compounds is called ____.a) hydrolysis b) electrolysis c) analysis d) synthesis

149. The reaction: methane (CH₄₎ + oxygen ---> carbon dioxide + water is an example of ________ reaction.a) double-replacementb) synthesis

c) complete combustiond) incomplete combustion

150. Which of the following reactions represents a single-replacement reaction?a) Ni + S ---> NiSb) 2H₂O ---> 2H₂ + O₂c) CuSO₄ + Fe ---> FeSO₄ + Cud) C + O₂ ---> CO₂

151. An example of a double-replacement reaction is ____.a) 2HgO ---> 2Hg + O₂b) Al₂(SO₄)₃ + 3Ca(OH)₂ ---> 2Al(OH)₃ + 3CaSO₄c) Zn + 2HCl ---> ZnCl₂ + H₂d) 3H₂ + N₂ ---> 2NH₃

152. The type of reaction represented by the generalized form of an equation: Y + BX ---> BY + X is a ____.a) synthesis reactionb) decomposition reaction

c) single-replacement reactiond) double-replacement reaction

153. All of the following reactions belong to one type <strong>except</strong>: a) 2NaCl ---> 2Na + Cl₂b) CaCO₃ --> CaO + O₂c) Ca(OH)₂ ---> CaO + H₂Od) Zn + H₂SO₄ ---> ZnSO₄ + H₂

154. The coefficient X which should appear when the following chemical equation is properly balanced? C₂H₆ + X O₂ ---> CO₂ + H₂Oa) 7b) 2

c) 8d) 6

e) None of the above.

155. The following is a combustion reaction. Balance and find the <strong>sum</strong> of the coefficients in the equation. C₃H₈ + oxygen ---> _______.a) 9b) 13

c) 15d) 16

e) None of the above.

156. Fluorine reacts with sodium hydroxide to form sodium fluoride, oxygen and water. What is the sum of the coefficients in the balanced chemical equation?a) 13 b) 17 c) 19 d) 21 e) 32

157. For the following single-replacement reaction, predict the reaction outcome and subsequent products: Mg + ZnCl₂ ---> ?a) No reaction.b) Yes, the reaction will proceed. Product is: MgZnClc) Yes, the reaction will proceed. Products are: Zn + MgCl₂d) Yes, the reaction will proceed. Products are: Zn + MgCl

158. Which of the following chemical equations correctly represents the reaction between aluminum and oxygen?a) 2Al(s) + 3O₂(g) ---> Al₂O₃(s)b) Al(s) + O₂(g) ---> AlO₂c) 3Al(s) + O₂ ---> Al₃O₂(s)d) 4Al(s) + 3O₂(g) ---> 2Al₂O₃(s)

159. What is the <strong>balanced</strong> <span style="text-decoration: underline;">net ionic equation</span> for the reaction of aqueous CaCl₂ and AgNO₃?a) CaCl₂(aq) + 2AgNO₃(aq) ---> Ca(NO₃)₂(aq) + 2AgCl(p)b) Ca²⁺(aq) + 2Cl^-(aq) + 2Ag⁺(aq) + 2NO₃^-(aq) ---> Ca²⁺(aq) + 2NO₃^-(aq) + 2AgCl(p)c) 2Cl^-(aq) + 2Ag⁺(aq) ---> 2AgCl(p)d) Cl^-(aq) + Ag⁺(aq) ---> AgCl(p)

160. Classify the following chemical reaction:2Al(s) + Fe₂O₃(s) ---> 2Fe(l) + Al₂O₃(s)a) synthesisb) decompositionc) combustiond) single-replacemente) double-replacement

161. What is the total number of atoms represented by the formula (NH₄)₂NaPO₄?a) 3 b) 7 c) 9 d) 16 e) 19

162. The term X in the correctly balanced chemical equation: 4NH₃ + 5O₂ ---> X + 6H₂O is _____.a) 2N2O b) 2N2O4 c) 4NO d) 2N2H4 e) 3NO2

163. Balance the chemical equation: FeS₂ + oxygen gas ---> Fe₂O₃ + sulfur dioxide. What is the coefficient for oxygen in the balanced chemical equation?a) 2b) 4

c) 7d) 11

e) None of the above.

164. What is the sum of all the coefficients in the complete combustion reaction of C₇H₁₆? C₇H₁₆ + O₂ ---> __________.a) 9 b) 16 c) 26 d) 27 e) 29

165. Predict the outcome of the reaction: HF(aq) + Cl₂(g) ---> ?a) No reaction.b) Yes, reaction will proceed. Products are HF(aq) + F₂(g).c) Yes, reaction will proceed. Products are HF(aq) + F(g).d) Yes, reaction will proceed. Product is HFCl(aq).

166. The reaction: Na⁺ + e^- --> Na⁰ is an example of:a) oxidation b) reduction c) synthesis d) combustion

167. The equation which represents a reduction is ______.a) H + OH- --> H2Ob) Cu⁰ --> Cu⁺² + 2e^-c) Fe⁺² - e^- --> Fe³⁺d) NaCl --> Na⁺ + Cl^-e) Br₂⁰ + 2e^- --> 2Br^-

168. Among the following Group 1 metals, the one most likely to oxidize is ____.a) cesium b) potassium c) sodium d) lithium

169. As the chlorine atom is reduced, the number of protone in its nucleus ______.a) increasesb) decreases

c) increases or decreases

d) stays the same

170. The oxidation number (sometimes also referred to as valence number) of an element indicates ______.a) its atomic massb) how many electrons its atom lends, borrow or sharesc) its stabilityd) what compounds it will form with other elements

171. The equation which represents an oxidation is ______.a) Cl⁰ + Cl⁰ --> Cl²b) Zn⁺² + 2e^- --> Znc) Fe⁺² - e^- --> Fe⁺³d) Na⁺ --> Na + e^-

172. When sulfur changes from an oxidation state of -2 to +6, it must _______.a) gain 2 electrons b) lose 6 electrons c) gain 4 electrons d) lose 8 electrons

173. Manganese to change from MnO₄^- to Mn⁺² must _____.a) gain 1 electron b) gain 5 electrons c) gain 3 electrons d) lose 1 electron

174. The gain of electrons by an atom, ion or group of atoms is ______.a) oxidation b) reduction c) electrolysis d) hydrolysis

175. In the reaction: AgNO₃ + NaCl --> NaNO₃ + AgCl, silver is ______.a) oxidized onlyb) reduced only

c) neither oxidized nor reducedd) both oxidized and reduced

176. Which compound has a middle element with the oxidation number of +6?a) Fe2(SO4)3 b) KMnO4 c) Ba(NO3)2 d) H2SO3

177. In the equation: 2Na + H₂ --> 2NaH, hydrogen is ____.a) oxidizedb) reduced

c) shows no change in its oxidation numberd) loses electrons

178. The formula that shows chlorine with an oxidation number of +7 is ____.a) HCl b) HClO2

- c) HClO3- d) HClO4

-

179. In the reaction: 2NO + O₂ --> 2NO₂, the oxidation number of nitrogen ____.a) changes from +2 to -2b) changes from +4 to +2

c) changes from +2 to +4d) is unchanged

180. In the reaction: 2H₂S + O₂ --> 2H₂O + 2S, which is the reducing agent?a) H2S b) O2 c) H2O d) S

181. Which is an example of an oxidation-reduction reaction?a) HCl + NaOH --> NaCl H₂Ob) CaCO₃ --> CaO + CO₂c) C + H₂O --> H₂ + COd) BaCl₂ + Na₂SO₄ --> 2NaCl + BaSO₄

182. Consider the following reaction in terms of oxidation-reduction. 1/2H₂(g) + 1/2F₂(g) --> HF(g) Which of the following is <strong>wrong</strong>?a) Hydrogen is oxidized by fluorine.b) Fluorine is reduced by oxygen.

c) The oxidation number of H₂ is zero.d) The oxidation number of fluorine in HF is +1.e) Oxidation number of F₂ is zero.

183. When sulfur dioxide is coverted into sulfur trioxide, each sulfur atom _____.a) is reducedb) gains one electron

c) loses three electronsd) has its oxidation number changed

184. In the following reaction: PbBr2 + 2KI --> PbI2 + 2KBr, ______________.a) PbBr2 is reducedb) PbBr2 is oxidized

c) KI is reducedd) PbBr2 is neither reduced nor oxidized

185. Assume that the order of decreasing activity of three non-metals (X, Y, and Z) is Y, Z, and X. It therefore follows that ______.a) Y cannot replace X from its compoundb) X can replace Y from its compound

c) Z can oxide X ions but not Y ionsd) Y can oxide X ions but not Z ions

----------Keys----------1. (d) 2. (e) 3. (c) 4. (c) 5. (e) 6. (d) 7. (e) 8. (a) 9. (c) 10. (a) 11. (b) 12. (d) 13. (b) 14. (c) 15. (b) 16. (b) 17. (c) 18. (e) 19. (a) 20. (d) 21. (c) 22. (d) 23. (b) 24. (a) 25. (a) 26. (b) 27. (b) 28. (d) 29. (a)

30. (b) 31. (c) 32. (b) 33. (e) 34. (b) 35. (d) 36. (d) 37. (a) 38. (e) 39. (e) 40. (c) 41. (c) 42. (a) 43. (d) 44. (c) 45. (b) 46. (b) 47. (b) 48. (c) 49. (d) 50. (a) 51. (c) 52. (a) 53. (e) 54. (c) 55. (a) 56. (a) 57. (a) 58. (d)

59. (c) 60. (b) 61. (c) 62. (b) 63. (d) 64. (b) 65. (c) 66. (b) 67. (c) 68. (a) 69. (c) 70. (b) 71. (e) 72. (d) 73. (e) 74. (b) 75. (c) 76. (b) 77. (c) 78. (d) 79. (c) 80. (a) 81. (a) 82. (d) 83. (d) 84. (c) 85. (a) 86. (b) 87. (b)

88. (b) 89. (b) 90. (d) 91. (c) 92. (c) 93. (c) 94. (d) 95. (a) 96. (c) 97. (c) 98. (d) 99. (d) 100. (c) 101. (d) 102. (c) 103. (b) 104. (d) 105. (a) 106. (a) 107. (c) 108. (d) 109. (a) 110. (d) 111. (b) 112. (c) 113. (d) 114. (b) 115. (a) 116. (c)

117. (c) 118. (b) 119. (a) 120. (e) 121. (a) 122. (b) 123. (e) 124. (b) 125. (d) 126. (b) 127. (a) 128. (d) 129. (b) 130. (b) 131. (a) 132. (c) 133. (d) 134. (a) 135. (b) 136. (c) 137. (c) 138. (a) 139. (c) 140. (a) 141. (d) 142. (a) 143. (b) 144. (b) 145. (c)

146. (a) 147. (c) 148. (d) 149. (c) 150. (c) 151. (b) 152. (c) 153. (d)

154. (a) 155. (b) 156. (a) 157. (c) 158. (d) 159. (d) 160. (d) 161. (d)

162. (c) 163. (d) 164. (d) 165. (a) 166. (b) 167. (e) 168. (a) 169. (d)

170. (b) 171. (c) 172. (d) 173. (b) 174. (b) 175. (c) 176. (a) 177. (b)

178. (d) 179. (c) 180. (b) 181. (c) 182. (d) 183. (d) 184. (d) 185. (c)